The compound with no dipole moment is -

Options

A. Methyl chloride
B. Carbon tetrachloride
C. Methylene chloride
D. Chloroform

Answer

To determine which compound has no dipole moment, we need to analyze the molecular structures of the given compounds and assess their symmetry and electronegativity differences.

### Step-by-Step Solution:

1. **Understanding Dipole Moment**:
- The dipole moment is a measure of the separation of positive and negative charges in a molecule. It is represented as \( \mu = q \times d \), where \( q \) is the charge and \( d \) is the distance between the charges.
- A molecule has a dipole moment if there is an unequal distribution of electron density, often due to differences in electronegativity between bonded atoms.

**Hint**: Remember that symmetrical molecules often have a net dipole moment of zero due to equal and opposite dipoles canceling each other out.

2. **Analyzing Methyl Chloride (CH3Cl)**:
- Structure: Tetrahedral with one chlorine atom and three hydrogen atoms.
- Electronegativity: Chlorine is more electronegative than carbon, leading to a dipole moment directed towards chlorine.
- Result: Methyl chloride has a net dipole moment.

**Hint**: Check for asymmetry in the molecular structure; if present, it likely has a dipole moment.

3. **Analyzing Carbon Tetrachloride (CCl4)**:
- Structure: Tetrahedral and symmetrical.
- Electronegativity: All four chlorine atoms are identical, and the symmetrical arrangement means that the dipoles cancel out.
- Result: Carbon tetrachloride has no net dipole moment.

**Hint**: Symmetrical molecules with identical atoms around a central atom typically have zero dipole moments.

4. **Analyzing Methylene Chloride (CH2Cl2)**:
- Structure: Tetrahedral with two chlorine atoms and two hydrogen atoms.
- Electronegativity: The dipoles from the C-Cl bonds do not cancel out due to the different electronegativities and the arrangement of atoms.
- Result: Methylene chloride has a net dipole moment.

**Hint**: Look for the number of different atoms and their arrangement; this can indicate whether dipoles will cancel.

5. **Analyzing Chloroform (CHCl3)**:
- Structure: Tetrahedral with one hydrogen and three chlorine atoms.
- Electronegativity: The dipoles from the C-Cl bonds do not fully cancel due to the presence of hydrogen.
- Result: Chloroform has a net dipole moment.

**Hint**: Consider how many different types of atoms are present and their positions; this affects the overall dipole moment.

### Conclusion:
The compound with no dipole moment is **Carbon Tetrachloride (CCl4)**.